For a solution formed by mixing liquids L and M, the vapour pressure of L plotted against the mole fraction of M in solution is shown in the following figure, Here x_(L) and x_(M) represent mole fraction of L and M, respectively in the solution, the correct statement(s) applicable to this system is (are) :

For a solution formed by mixing liquids L and M, the vapour pressure o

1.	For a solution formed by mixing liquids L and M, the vapour pressure of L plotted against the mole fraction of M in solution is shown in the following figure, Here x_(L) and x_(M) represent mole fraction of L and M, respectively in the solution, the correct statement(s) applicable to this system is (are) :
Answer» ATTRACTIVE intramolecular interactions between L-L in pure liquid L and M-M in pure liquid M are stronger than those between L-M when MIXED in solution The point Z represents vapour pressure of pure liquid M and Raoult's law is obeyed when `x_(L) rarr 0` The point Z represents vapour pressure of pure liquid L and Raoult's law is obeyed when `x_(L) rarr1` The point Z represents vapour pressure of pure liquid M and Raoult's is law is obeyed from `x_(L) = 0` to `x_(L) =1` Solution :Graph shows positive deviation from Raoult's law hence INTERMOLECULAR force must be less in solution as compared to pure liquids `F_(L-L),F_(M-M)gt F_(L-M)` (SEQUENCE of intermolecular force) At point Z `p_(L) = p_(L)^(0)x_(L)` When `x_(M)=0`, then `x_(L)=1` `:. p_(L) = p_(L)^(0)`= pure liquid L]